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Prelim paper
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1
Name
Register Number Class
SCIENCE CHEMISTRY 5116/3
Paper 3
MAY 2010 1 hour 15 minutes
PRELIMINARY EXAMINATION
SECONDARY FOUR EXPRESS/SECONDARY FIVE NORMAL
READ THESE INSTRUCTIONS FIRST
Do not open this booklet until you are told to do so. Write your name, class and register number on top of this page and on any separate answer paper used. Section A Answer all questions. Write down your answers in the space provided in the answer sheet. Section B Answer 2 out of 3 questions. Write down your answers on the answer sheet provided. At the end of the examination: Hand in the Answer sheet only .
For Examiner’s Use Section A Section B TOTAL
[Turn over
This question paper consists of 11 printed pages.
MACPHERSON SECONDARY SCHOOL
2
Section A (45 Marks)
Answer all the questions in the answer booklet provided.
A1 The diagram below shows the structure of an atom of element Q.
(a) Complete the table below about the three different particles found in an atom of element Q.
Particle Name of particle Relative charge
X
(b) Is element Q a metal or non-metal? Give a reason for your answer.
(c) Element Q reacts with oxygen to form the compound Q2O.
(i) Draw a dot-and-cross diagram of the electronic structure of the compound. Show only the outer electrons. (ii) Would you expect the compound to have a high or low melting point ? Explain your answer.
[3] [1] [3] [2]
●
○
3
A2 Carbon monoxide reacts with copper (II) oxide accordng to the following equation:
CO + CuO CO2 + Cu
(a) What volume of cabon monoxide is required to to convert 4.0 g of copper (II) oxide [2]
(b) Find the mass of copper metal obtained at the end of the reaction. [2]
(c) Find the number of moles of carbon dioxide molecules produced under room conditions.
[2]
A3 Given below is a list of substances.
Sodium hydroxide Silver Chloride Magnesium Lead (II) nitrate
Dilute nitric acid Calcium oxide Ammonium sulfate
Select from the list above, substance(s) that is suitable for the following descriptions.
(a)
A salt that is prepared by precipitation.
(b)
Two substances that are reacted to form magnesium nitrate.
(c)
A substance that is prepared by titration.
(d)
A substance that is added to neutralise the soil.
(e)
Two substances when reacted in the aqueous state forms a white preciptate that dissolves when one of the reactant is added in excess.
(f) A substance that can liberate a gas that turns damp red litmus blue
[6]
4
A4
(a) Deduce the identity of the substance lettered M, P, Q, R and S by giving their chemical name.
[5]
(b) Write down the equation for the reaction of metal M with dilute hydochloric acid. [2]
(c) Describe how you can identify the combustible gas. [2]
A5
Answer the following questions using the metals below:
copper zinc magnesium sodium iron
(a) Name the most reactive metal
(b) Write down the name of the metal which is likely to be found native (i.e. naturally occurring).
(c) Which metal does not react with water but reacts readily with dilute
hydrochloric acid.
(d) Which metal is used to galvanise iron sheets.
[1] [1] [1] [1]
5
A6 The figure below shows an experiment to be carried out by a student to investigate the substances formed when methane burns in plentiful supply of air.
a) A liquid P collects in tube A. Name liquid P. [1]
b) What would you expect to see in tube B during the experiment? [1]
c) Write a balanced chemical equation for the complete combustion of
methane in air. [1]
d) However, if insufficient air is present, a different colourless gas is produced in the combustion. This gas could be harmful to the student.
i) Name this substance. [1]
ii) How might the gas be harmful to the student? [1]
[Turn over
6
A7
An experiment was set up as shown in the diagram below. It investigated the reaction between granulated zinc and 2.0 mol/dm3 sulphuric acid. The results of the experiment are shown in the graph below.
granulated zinc
sulphuric acid
(i) On the same axes above, sketch what you would expect if the experiment was repeated at a lower temperature.Label the curve T.
(ii) On the same axes above, sketch what you would expect
if the experiment was repeated using zinc powder. Label the curve P .
(iii) In terms of the kinetic particle theory (the movement of
particles of matter), explain the effect of a higher temperature on the speed of reaction.
[2] [2] [2]
[Turn over
7
SECTION B (10 marks each) Answer TWO essay questions only
B1 (a) Although sodium chloride and butane have approximately the same relative molecular mass, the boiling point of sodium chloride is more than 1000oC higher than that of butane. With the aid of suitable diagrams, explain why the boiling point of sodium chloride is much higher than that of butane.
[5]
B1(b) Uranium is between magnesium and zinc in the reactivity series.
Equal sized strips of magnesium, uranium and zinc were placed in hydrochloric acid.
The hydrochloric acid was of the same concentration. The results are shown in the table.
(i) Describe the observation of uranium with hydrochloric acid.
(ii) Uranium has several isotopes which are radioactive.
One of its isotopes is uranium–235. The other is Uranium –237.
What do you understand by the term isotopes?
How do these two isotopes differ?
[2] [3]
8
B2(a) There are three main stages involved in the production of polythene bottles from crude oil. Polythene is also known as polyethene.
(i) State the processes involved in :
how heavy oil can be obtained from crude oil in stage I. how monomer X be obtained from heavy oil in stage II.
[2]
(ii) Draw the structure of monomer X.
[2]
(iii) Describe a test to confirm the nature of monomer X.
[2]
) B2(b)B2(b)
The macromolecule below is an addition polymer.
Polymer X
(i) Draw the structure of the monomer from which polymer X is formed.
(ii) Polymer X is used as an insulating cover for electrical wires. Explain why polymer X does not conduct electricity.
(iii) Polymer X is non-biodegradable. Describe one pollution problem that this causes.
[Turn over
[2] [1] [1]
Crude oil Heavy oil Monomer X
Polythene bottles
Stage I Stage II Stage III
C C C C C C
H H H H H H
H H Cl H Cl Cl
9
B3
An experiment was carried out to investigate the rate of decomposition of aqueous hydrogen peroxide at room temperature. The unbalanced equation and the total volume of oxygen gas given off every twenty seconds is given below.
H2O2 (aq) → H2O (l) + O2 (g)
Time / s 0 20 40 60 80 100 120 140 160 Total volume of oxygen /cm3
0
14
22
33
35
36
36
36
(a) Copy and balance the chemical equation above. [1]
(b) Plot the graph of total volume of oxygen against time on the graph paper provided in the answer sheet.
Use the graph that you have plotted , to
i) estimate the missing the volume of oxygen at 60 seconds.
ii) state the total volume of oxygen produced at the end of reaction.
[3] [1] [1]
(c) Describe how you can test for the gas evolved .
[2]
(d) The reaction was repeated at 800C. Sketch and label on the same graph paper, the graph for the reactions
carried out for this temperatures.
[2]
#### END OF PAPER THREE#####
10
DATA SHEET The Periodic Table of Elements
Group I II III IV V VI VII 0
1
H Hydrogen
1
4
He Helium
2
7
Li Lithium
3
9
Be Beryllium
4
11
B Boron
5
12
C Carbon
6
14
N Nitrogen
7
16
O Oxygen
8
19
F Fluorine
9
20
Ne Neon
10
23
Na Sodium
11
24
Mg Magnesium 12
27
Al Aluminium
13
28
Si Silicon
14
31
P Phosphorus 15
32
S Sulphur
16
35.5
Cl Chlorine 17
40
Ar Argon
18
39
K Potassium 19
40
Ca Calcium
20
45
Sc Scandium
21
48
Ti Titanium 22
51
V Vanadium 23
52
Cr Chromium
24
55
Mn Manganese 25
56
Fe Iron
26
59
Co Cobalt
27
59
Ni Nickel
28
64
Cu Copper
29
65
Zn Zinc
30
70
Ga Gallium
31
73
Ge Germanium 32
75
As Arsenic
33
79
Se Selenium
34
80
Br Bromine
35
84
Kr Krypton
36
85
Rb Rubidium 37
88
Sr Strontium
38
89
Y Yttrium
39
91
Zr zirconium 40
93
Nb Niobium
41
96
Mo Molybdenum
42
Tc Technetium 43
101
Ru Ruthenium
44
103
Rh Rhodium
45
106
Pd Palladium 46
108
Ag Silver
47
112
Cd Cadmium 48
115
In Indium
49
119
Sn Tin
50
122
Sb Antimony
51
128
Te Tellurium
52
127
I Iodine
53
131
Xe Xenon
54
133
Cs Caesium
55
137
Ba Barium
56
139
La Lanthanum 57
178
Hf Hafnium
72
181
Ta Tantalum 73
184
W Tungsten
74
186
Re Rhenium
75
190
Os Osmium
76
192
Ir Iridium
77
195
Pt Platinum
78
197
Au Gold
79
201
Hg Mercury
80
204
Tl Thallium
81
207
Pb Lead
82
209
Bi Bismuth
83
Po Polonium
84
At Astatine
85
Rn Radon
86
Fr Francium 87
226
Ra Radium
88
227
Ac Actinium
89
*58-71 Lanthanoid series †90-103 Actinoid series
140
Ce Cerium
58
141
Pr Praseodymium 59
144
Nd Neodymium 60
Pm Promethium 61
150
Sm Samarium 62
152
Eu Europium 63
157
Gd Gadolinium 64
159
Tb Terbium
65
162
Dy Dysprosium 66
165
Ho Holmium
67
167
Er Erbium
68
169
Tm Thulium
69
173
Yb Ytterbium 70
175
Lu Lutetium
71
a
X b
A = relative atomic mass
X = atomic symbol
B = proton (atomic) number
232
Th Thorium
90
Pa Protactinium
91
238
U Uranium
92
Np Neptunium
93
Pu Plutonium 94
Am Americium 95
Cm Curium
96
Bk Berkelium 97
Cf Californium 98
Es Einsteinium 99
Fm Fermium
100
Md Mendelevium
101
No Nobelium 102
Lr Lawrencium 103
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.)
11
Colours of Some Common Metal Hydroxides
Calcium hydroxide White Copper(II) hydroxide Light blue
Iron(II) hydroxide Green Iron(III) hydroxide Red-brown Lead(II) hydroxide White
Zinc hydroxide White